Cambridge IGCSE™
CHEMISTRY0620/01
Paper 1 Multiple Choice (Core)
For examination from 2023
45 minutes
SPECIMEN PAPER
You must answer on the multiple choice answer sheet.
*0123456789*
You will need:
Multiple choice answer sheet
Soft clean eraser
Soft pencil (type B or HB is recommended)
INSTRUCTIONS
●
There are forty questions on this paper. Answer all questions.
●
For each question there are four possible answers A, B, C and D. Choose the one you consider correct
and record your choice in soft pencil on the multiple choice answer sheet.
●
Follow the instructions on the multiple choice answer sheet.
●
Write in soft pencil.
●
Write your name, centre number and candidate number on the multiple choice answer sheet in the
spaces provided unless this has been done for you.
●
Do not use correction fluid.
●
Do not write on any bar codes.
●
You may use a calculator.
INFORMATION
●
The total mark for this paper is 40.
●
Each correct answer will score one mark.
●
Any rough working should be done on this question paper.
●
The Periodic Table is printed in the question paper.
This document has 16 pages. Any blank pages are indicated.
© UCLES 2020
[Turn over
2
1
2
Which statement about liquids and gases is correct?
A
1 cm3 of gas contains more particles than 1 cm3 of liquid.
B
A given mass of liquid has a fixed volume at room temperature.
C
Particles in a liquid can easily be forced closer together.
D
Particles in a liquid have fixed positions.
Mineral wool soaked in aqueous ammonia is placed in the apparatus shown.
mineral wool soaked
in aqueous ammonia
damp red
litmus paper
After five minutes, the damp red litmus paper turns blue.
Which process led to this change?
3
4
A
condensation
B
crystallisation
C
diffusion
D
distillation
Which pair of atoms contains the same number of neutrons?
A
59
Co
27
and
59
Ni
28
B
64
Cu
29
and
65
Cu
29
C
64
Cu
29
and
65
Zn
30
D
65
Cu
29
and
65
Zn
30
Which statement describes the bonding in sodium chloride?
A
A shared pair of electrons between two atoms leading to a noble gas configuration.
B
A strong force of attraction between oppositely charged ions.
C
A strong force of attraction between two molecules.
D
A weak force of attraction between oppositely charged ions.
© UCLES 2020
0620/01/SP/23
3
5
A covalent molecule M contains a total of four shared electrons.
What is M?
6
A
ammonia, NH3
B
hydrogen chloride, HCl
C
methane, CH4
D
water, H2O
The ‘lead’ in a pencil is made of a mixture of graphite and clay.
‘lead’
When the percentage of graphite is increased, the pencil moves across the paper more easily.
Which statement explains this observation?
7
A
Graphite has a high melting point.
B
Graphite is a form of carbon.
C
Graphite is a lubricant.
D
Graphite is a non-metal.
A compound with the formula XO2 has a relative formula mass of 64.
What is X?
A
cadmium
B
copper
C
gadolinium
D
sulfur
© UCLES 2020
0620/01/SP/23
[Turn over
4
8
9
When molten lead(II) bromide is electrolysed using platinum electrodes, what is observed at each
electrode?
negative electrode
positive electrode
A
bubbles of a colourless gas
bubbles of a brown gas
B
bubbles of a colourless gas
bubbles of a colourless gas
C
shiny grey liquid
bubbles of a brown gas
D
shiny grey liquid
bubbles of a colourless gas
Aqueous nickel(II) sulfate is used as the electrolyte to electroplate a piece of steel with nickel.
Which materials are used as the negative electrode and positive electrode?
negative electrode
positive electrode
A
carbon
steel
B
nickel
steel
C
platinum
nickel
D
steel
nickel
10 Which row shows the waste products released from the exhaust of a vehicle powered using a
hydrogen–oxygen fuel cell?
carbon dioxide
oxides of nitrogen
water
A



B



C



D



© UCLES 2020
0620/01/SP/23
5
11
A reaction pathway diagram is shown.
products
energy
reactants
progress of reaction
Which statement about the reaction is correct?
A
Heat is released.
B
It is a combustion reaction.
C
It is an endothermic reaction.
D
The temperature increases.
12 Which changes are physical changes?
A
1
melting ice to form water
2
burning hydrogen to form water
3
adding sodium to water
4
boiling water to form steam
1 and 2
© UCLES 2020
B
1 and 4
C
2 and 3
0620/01/SP/23
D
3 and 4
[Turn over
6
13 The diagram shows an experiment to measure the rate of a chemical reaction.
dilute
hydrochloric acid
measuring cylinder
metal
water
Which change decreases the rate of reaction?
A
adding water to the flask
B
heating the flask during the reaction
C
using more concentrated acid
D
using powdered metal
14 Which row correctly matches the experiment and observations to the identity of the underlined
substance?
experiment and observations
identity of the underlined substance
A
Blue crystals are heated.
The crystals turn white and steam is given off.
hydrated cobalt(II) chloride
B
Pink crystals are heated.
The crystals turn blue and steam is given off.
anhydrous cobalt(II) chloride
C
Water is added to a blue solid.
The blue solid turns pink.
hydrated copper(II) sulfate
D
Water is added to a white solid.
The white solid turns blue.
anhydrous copper(II) sulfate
15 Which equation shows an oxidation reaction?
A
C + O2 → CO2
B
CaCO3 → CaO + CO2
C
CaO + 2HCl → CaCl 2 + H2O
D
N2O4 → 2NO2
© UCLES 2020
0620/01/SP/23
7
16 Farmers spread calcium hydroxide on their fields to neutralise soils that are too acidic for crops to
grow well.
Which ion neutralises the acid in the soil?
A
Ca2+
B
H+
O2–
C
D
OH–
17 Four different solutions, J, K, L and M, are tested with universal indicator.
solution
J
K
L
M
colour with
universal indicator
green
red
purple
orange
Which solutions are acidic?
A
J and M
B
C
K and M
D
K only
L only
18 Period 3 of the Periodic Table is shown.
Na
Mg
Al
Si
P
S
Cl
Ar
What increases from Na to Ar across Period 3?
A
density
B
melting point
C
non-metallic character
D
the number of electron shells
19 Sodium and rubidium are elements in Group I of the Periodic Table.
Which statement is correct?
A
Sodium atoms have more electrons than rubidium atoms.
B
Sodium has a lower density than rubidium.
C
Sodium has a lower melting point than rubidium.
D
Sodium is more reactive than rubidium.
© UCLES 2020
0620/01/SP/23
[Turn over
8
20 Chlorine, bromine and iodine are elements in Group VII of the Periodic Table.
Which statement about these elements is correct?
A
The colour gets lighter down the group.
B
The density decreases down the group.
C
They are all gases at room temperature and pressure.
D
They are all non-metals.
21 Which row describes the properties of a typical transition element?
melting point
forms coloured
compounds
can act as a
catalyst
A
high
no
no
B
high
yes
yes
C
low
no
yes
D
low
yes
no
22 Which statement about the noble gases is correct?
A
Noble gases are diatomic molecules.
B
Noble gases are reactive gases.
C
Noble gases have full outer electron shells.
D
The noble gases are found on the left-hand side of the Periodic Table.
23 What is a property of all metals?
A
conducts electricity
B
hard
C
low melting point
D
reacts with water
24 Which statement explains why aluminium is used in the manufacture of aircraft?
A
It conducts heat well.
B
It has a low density.
C
It is a good insulator.
D
It is easy to recycle.
© UCLES 2020
0620/01/SP/23
9
25 Which diagram represents a solid alloy?
A
B
C
D
26 Metals W, X, Y and Z are reacted with dilute hydrochloric acid.
The oxides of metals W, X, Y and Z are heated with carbon.
The results are shown.
reaction
W
X
Y
Z
metal + dilute
hydrochloric acid
fizzing
fizzing
violent fizzing
no reaction
metal oxide +
carbon and heat
no reaction
metal
produced
no reaction
metal
produced
What is the order of reactivity of the metals?
most reactive
least reactive
A
Y
W
X
Z
B
Y
X
W
Z
C
Z
W
X
Y
D
Z
X
W
Y
© UCLES 2020
0620/01/SP/23
[Turn over
10
27 The diagrams show experiments involving the rusting of iron.
test-tube P
test-tube Q
test-tube R
oil
iron nails
water
water boiled to
remove the air
anhydrous
calcium chloride
to dry the air
A student predicted the following results.
1
In test-tube P, the iron nails rust.
2
In test-tube Q, the iron nails do not rust.
3
In test-tube R, the iron nails do not rust.
Which predictions are correct?
A
1, 2 and 3
B
1 and 2 only
C
1 and 3 only
D
2 and 3 only
28 Which statement about the extraction of iron in a blast furnace is correct?
A
Calcium oxide reacts with basic impurities.
B
Carbon is burnt to provide heat.
C
Iron(III) oxide is reduced to iron by carbon dioxide.
D
The raw materials are bauxite, limestone and coke.
29 Which process is used to convert calcium carbonate into calcium oxide?
A
electrolysis
B
fractional distillation
C
incomplete combustion
D
thermal decomposition
© UCLES 2020
0620/01/SP/23
11
30 Which substance is beneficial to aquatic life?
A
dissolved oxygen
B
phosphates
C
plastics
D
sewage
31 A new planet has been discovered and its atmosphere has been analysed.
atmosphere
planet
The table shows the composition of its atmosphere.
gas
percentage by volume
carbon dioxide
4
nitrogen
72
oxygen
24
Which gases are present in the atmosphere of the planet in a higher percentage than they are in
the Earth’s atmosphere?
A
carbon dioxide and oxygen
B
carbon dioxide only
C
nitrogen and oxygen
D
nitrogen only
32 Which statement is correct?
A
Atmospheric carbon dioxide is not a cause of climate change.
B
Atmospheric methane is produced by respiration.
C
Burning natural gas decreases the level of carbon dioxide in the atmosphere.
D
Decomposition of vegetation causes an increase in atmospheric methane.
© UCLES 2020
0620/01/SP/23
[Turn over
12
33 A plastic combusts to form sulfur dioxide, SO2, and hydrogen chloride, HCl.
How could both gases be removed from the air?
A
Pass the gases over solid anhydrous cobalt(II) chloride.
B
Pass the gases over solid damp calcium oxide.
C
Pass the gases through a catalytic converter.
D
Pass the gases through filter paper.
34 Limestone fizzes and dissolves in dilute hydrochloric acid.
What is the word equation for this reaction?
A
calcium carbonate + hydrochloric acid → calcium chloride + carbon dioxide
B
calcium carbonate + hydrochloric acid → calcium chloride + water + carbon dioxide
C
calcium hydroxide + hydrochloric acid → calcium chloride + hydrogen
D
calcium oxide + hydrochloric acid → calcium chloride + water
35 Three equations involving organic compounds are shown.
C4H10 → C2H4 + C2H6
C2H4 + H2O → C2H5OH
C2H5OH + 3O2 → 2CO2 + 3H2O
How many different homologous series are shown in these equations?
A
1 B
2
C
3
D
4
36 Petroleum is a mixture of different hydrocarbons.
Which process is used to separate the petroleum into groups of similar hydrocarbons?
A
combustion
B
cracking
C
fractional distillation
D
reduction
© UCLES 2020
0620/01/SP/23
13
37 Ethene is a hydrocarbon.
Which row shows the type of covalent bond between the carbon atoms in ethene and the effect of
ethene on aqueous bromine?
type of covalent bond
effect of ethene on aqueous bromine
A
single bond
colour changes from brown to colourless
B
single bond
colour changes from colourless to brown
C
double bond
colour changes from brown to colourless
D
double bond
colour changes from colourless to brown
38 Which statements about ethanoic acid are correct?
A
1
It turns universal indicator purple.
2
It reacts with magnesium to form hydrogen gas.
3
It reacts with calcium carbonate to form carbon dioxide gas.
4
It decolourises aqueous bromine.
1, 2 and 3
B
1 and 2 only
C
2, 3 and 4
D
2 and 3 only
39 Five steps in an acid–base titration are shown.
1
Slowly add the acid from a burette into a conical flask until the indicator becomes
colourless.
2
Add thymolphthalein.
3
Use a volumetric pipette to add a fixed volume of alkali to a conical flask.
4
Read and record the initial volume of acid in the burette.
5
Read and record the final volume of acid in the burette.
What is the correct order of these steps to complete an acid–base titration?
A
2 → 4 → 1 → 5 → 3
B
3 → 2 → 4 → 1 → 5
C
3 → 4 → 1 → 5 → 2
D
4 → 3 → 1 → 2 → 5
© UCLES 2020
0620/01/SP/23
[Turn over
14
40 The chromatogram obtained from four mixtures of dyes, P, Q, R and S, is shown.
solvent front
baseline
P
Q
R
S
What is the total number of different dyes identified in the four mixtures?
A
3 © UCLES 2020
B
4
C
5
0620/01/SP/23
D
8
© UCLES 2020
12
Sc
Ti
V
Cr
Mn
Co
27
Ni
28
Cu
29
Zn
30
0620/01/SP/23
104
88
–
90
89
232
thorium
actinium
–
Th
Ac
140
cerium
139
lanthanum
59
231
protactinium
Pa
91
141
praseodymium
Pr
–
58
Ce
–
Db
dubnium
Rf
rutherfordium
La
57
actinoids
105
181
tantalum
Ta
73
93
Nb
niobium
41
51
vanadium
238
uranium
U
92
144
neodymium
60
Nd
–
Sg
seaborgium
106
184
tungsten
W
74
96
Mo
molybdenum
42
52
chromium
–
neptunium
Np
93
–
promethium
61
Pm
–
Bh
bohrium
107
186
rhenium
Re
75
–
Tc
technetium
43
55
manganese
Fe
–
plutonium
Pu
94
150
samarium
62
Sm
–
Hs
hassium
108
190
osmium
Os
76
101
Ru
ruthenium
44
56
iron
–
americium
Am
95
152
europium
63
Eu
–
Mt
meitnerium
109
192
iridium
Ir
77
103
Rh
rhodium
45
59
cobalt
–
curium
Cm
96
157
gadolinium
64
Gd
–
Ds
darmstadtium
110
195
platinum
Pt
78
106
Pd
palladium
46
59
nickel
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
actinoids
lanthanoids
–
Ra
radium
Fr
francium
89–103
178
87
137
hafnium
133
barium
Hf
caesium
lanthanoids
Ba
72
91
Zr
zirconium
40
48
titanium
Cs
89
57–71
88
56
85
55
Y
yttrium
Sr
strontium
39
45
Rb
38
40
Ca
rubidium
37
39
K
scandium
–
berkelium
Bk
97
159
terbium
65
Tb
–
Rg
roentgenium
111
gold
197
Au
79
108
silver
Ag
47
64
copper
–
californium
Cf
98
163
dysprosium
66
Dy
–
Cn
copernicium
112
201
mercury
Hg
80
112
Cd
cadmium
48
65
zinc
calcium
26
potassium
25
31
24
–
einsteinium
Es
99
165
holmium
67
Ho
–
Nh
nihonium
113
204
thallium
Tl
81
115
In
indium
49
70
gallium
Ga
27
20
24
19
23
aluminium
Al
13
11
boron
magnesium
23
1
sodium
22
B
C
N
7
O
8
VI
F
9
VII
2
VIII
–
fermium
Fm
100
167
erbium
68
Er
–
Fl
flerovium
114
lead
207
Pb
82
119
tin
Sn
50
73
Ge
germanium
32
28
silicon
Si
14
12
carbon
–
mendelevium
Md
101
169
thulium
69
Tm
–
Mc
moscovium
115
209
bismuth
Bi
83
122
Sb
antimony
51
75
As
arsenic
33
31
phosphorus
P
15
14
nitrogen
–
nobelium
No
102
173
ytterbium
70
Yb
–
Lv
livermorium
116
–
polonium
Po
84
128
Te
tellurium
52
79
Se
selenium
34
32
sulfur
S
16
16
oxygen
–
Lr
lawrencium
103
175
lutetium
71
Lu
–
Ts
tennessine
117
–
astatine
At
85
127
I
iodine
53
80
Br
bromine
35
35.5
chlorine
Cl
17
19
fluorine
–
oganesson
Og
–
118
radon
86
Rn
131
Xe
xenon
54
84
Kr
krypton
36
40
argon
18
Ar
20
neon
Ne
10
4
helium
6
V
hydrogen
5
IV
He
Mg
21
relative atomic mass
name
atomic symbol
atomic number
Key
III
H
1
Na
9
11
7
Be
beryllium
Li
4
3
lithium
II
I
Group
The Periodic Table of Elements
15
16
BLANK PAGE
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
Cambridge Assessment International Education is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of the University of
Cambridge Local Examinations Syndicate (UCLES), which itself is a department of the University of Cambridge.
© UCLES 2020
0620/01/SP/23